CHEM 120 Chapter Notes - Chapter 4: Kinetic Theory Of Gases, Pressure Measurement, Ideal Gas Law
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CHEM 120 Full Course Notes
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Adopts the shape of the (cid:272)o(cid:374)tai(cid:374)er to the e(cid:454)te(cid:374)t of the (cid:272)o(cid:374)tai(cid:374)er"s (cid:448)olu(cid:373)e. parti(cid:272)les far apart and move randomly. Gases have relatively low densities compared to solids/liquids. When a gas cools, its density increases because its volume decreases. Adopts shape of co(cid:374)tai(cid:374)er to the e(cid:454)te(cid:374)d of the co(cid:374)tai(cid:374)er"s volu(cid:373)e. particles close together but free to move around each other. Particles close together and held rigidly in place. The force of gravity attracts atmospheric gases and they exert a force uniformly on all surfaces. If the pressures from outside and inside a body are not equal, the shape of the objects changes. At sea level and under ordinary atmospheric conditions = 760mm. The (cid:449)eight of (cid:373)er(cid:272)ur(cid:455) (cid:449)ould (cid:271)e greater i(cid:374) a wider tub, but so is the area. Thus, the pressure(the ratio of weight to area) is the same. Used to measure pressure of gases in experiments. Units: 1 atm = 101. 325 kpa = 1. 01325*105 pa.